Correct statbility order of metal cation is /are :

Options

A. `Pb^(2+) lt Sn^(2+)`
B. `Pb^(4+) lt Pb^(2+)`
C. `Sn^(4+) lt Sn^(2+)`
D. `Pb^(4+) lt Sn^(4+)`

Explanation

To determine the correct stability order of metal cations, we need to analyze the oxidation states of tin (Sn) and lead (Pb), which belong to the carbon family (Group 14 of the periodic table).

### Step-by-Step Solution:

1. **Identify the Elements**:
- The elements in question are tin (Sn) and lead (Pb), which are part of the carbon family (Group 14).

2. **Understand the Oxidation States**:
- Both tin and lead can exhibit oxidation states of +2 and +4.
- For example, Sn can exist as Sn²⁺ and Sn⁴⁺, while Pb can exist as Pb²⁺ and Pb⁴⁺.

3. **Consider the Electron Configuration**:
- The outermost electronic configurations for Sn and Pb are:
- Sn: [Kr] 5s² 4d¹⁰ 5p²
- Pb: [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p²

4. **Inert Pair Effect**:
- As we move down the group from Sn to Pb, the inert pair effect becomes significant. This effect refers to the tendency of the s-electrons (the two electrons in the outermost s-orbital) to remain non-bonding or inert.
- This means that the +2 oxidation state becomes more stable compared to the +4 oxidation state as we go down the group.

5. **Stability Order**:
- For Sn, the +2 state (Sn²⁺) is more stable than the +4 state (Sn⁴⁺).
- For Pb, the +2 state (Pb²⁺) is also more stable than the +4 state (Pb⁴⁺).
- Therefore, the stability order can be summarized as:
- Sn²⁺ > Sn⁴⁺
- Pb²⁺ > Pb⁴⁺

6. **Conclusion**:
- The correct stability order of metal cations for Sn and Pb is:
- +2 oxidation state is more stable than +4 for both Sn and Pb.
- Thus, the correct options are B (+2 is more stable than +4) and D (Sn⁴⁺ is more stable than Pb⁴⁺).

### Final Answer:
- The correct stability order of metal cations is:
- B: +2 is more stable than +4
- D: Sn⁴⁺ is more stable than Pb⁴⁺